1. Chemistry: The Big Picture
What impact does chemistry have on our everyday lives?
How does the structure of individual atoms determine their behavior in all types of matter?
What mathematical relationships can be used to predict the interaction of matter?
How do environmental conditions affect the interactions of matter?

2. Final Exam BIG Topics What do you know? What do you need to know?
Atomic Structure (structure/isotopes) & Nuclear Chemistry
Electrons in Atoms (electron configurations/equations)
Periodic Table/Periodic Trends
Chemical Bonding (Ionic/Molecular/Metallic)
Lewis Structures/Electron Geometry/Molecular Geometry
Organic Chemistry
Types of Reactions, Net Ionic Equations, Reaction Stoichiometry, Limiting Reagent
States of Matter, Gas Laws
Water & Aqueous Systems (Solutions/Colligative Properties)
Thermochemistry
Reaction Rates & Chemical Equilibrium
Acids & Bases

3. Big Problems Items Nuclear Reactions Electron configurations
Math of an electron
Organic Chemistry
Chemical Reactions
Net Ionic Equation
Stoichiometry/Limiting Reagent
Chemical Equilibrium (Keq or Ksp)
Acid or Base Dissociation (Ka or Kb)
Freezing Pt Depression or Boiling Pt Elevation
Hess Law
Titration
Thermochemistry
Gas Laws

4. Chemical Formulas Topics: Balanced chemical reactions, net ionic equations, oxidation reduction
Can you determine the molar mass of these substances?
Can you draw a VSEPR model of a water molecule?
Water
Sodium nitrate
Copper (II) carbonate
Iron (III) bromide
Hydrochloric acid
Carbonic acid
Sodium hydroxide
Can you identify the substances as an acid, base, salt, ionic or molecular?
Can you combine the components and write balanced chemical reactions?

5. Chemical Names
MgSO4
HBr
NaOH
NH3
CuS

6. Net Ionic Equations
A student reacts aqueous barium nitrate and aqueous sodium sulfate in a test tube.
Balance the occurring chemical reaction.
Write the net ionic equation.
Identify the spectator ions.

7. Composition Stoichiometry Activity
Complete A-F with the correct conversion factor. A B F C D E

8. Composition Stoichiometry
What is the number of moles in 432 g Ba(NO3)2 ?
How many atoms are in 3.25 grams of calcium carbonate?

9. Stoichiometric Calculations
The figure below summarizes the steps for a typical stoichiometric problem.

10. Reaction Stoichiometry
Diagraming the process for the following types of problems
Mole-mole (Always used to solve Rxn Stoic problems)
Mass-mole
Mole-Mass
Mass-Mass
Mass-Volume
Volume-Mole

11. Reaction Stoichiometry
Iron( III) oxide is formed when iron combines with oxygen in the air. How many grams of Fe O are formed when 16.7 g of Fe reacts completely with oxygen?
___Fe (s) + ___O2 (g)  ___Fe2O3 (s)

12. _____N2 + _____H2  _____NH3
Limiting Reactant
How many grams of NH3 can be produced from the reaction of 96 g of N2 and 32.1 g of H2?
_____N2 + _____H2  _____NH3

13. Molecular formula
Determine the molecular formula of a compound with the empirical formula of C2H4O and molar mass of 88g.

14. Using the data shown in the diagram, determine the value for P2.
75 kPa
660 kPa
130 kPa
21 kPa
150 kPa

15. Gas Laws
How many moles of N2 are in a flask with a volume of 250 mL at a pressure of 3 atm and a temperature of K?

16. Colligative properties
Calculate the freezing point of 50.0 g of water if grams of NaCl is added to the water.

17. Thermochemistry
If heat is released by a chemical system, an equal amount of heat will be ____. a.
absorbed by the surroundings c.
released by the surroundings b.
absorbed by the universe d.
released by the universe

18. Thermochemistry
How much heat (in kJ) is released or absorbed when mol of sodium bicarbonate is decomposed according to the reaction below?
2NaHCO3(s)  Na2CO3(s) + H2O(g)+ CO2(g) H =129 kJ

19. Thermochemistry
Calculate H for the reaction of sulfur dioxide with oxygen. 2SO2 (g) + O2 (g)  2SO3 (g) ( H SO2 (g) = –296.8 kJ/mol;  H SO3 (g) = –395.7 kJ/mol)

20. Thermochemistry: Hess’s Law
PbCl2(s) + Cl2(g) → PbCl4(l) ΔH = ?
Pb(s) + 2Cl2(g) → PbCl4(l) ΔH = kJ
Pb(s) + Cl2­(g) → PbCl2(s) ΔH = kJ

21. Factors Affecting Equilibrium: Le Châtelier’s Principle
Le Châtelier’s Principle (Henri Le Chatelier ( ))
Stresses that upset the equilibrium of a chemical system include
changes in the concentration of reactants or products
changes in temperature
changes in pressure
Le Châtelier’s principle: If a stress is applied to a system in dynamic equilibrium, the system changes in a way that relieves the stress.

22. Equilibrium Constants
Liquids & Solids are somewhat isolated. They are not included in the Keq equation. They are treated as a “1” value.
Equilibrium Constants
The equilibrium constant (Keq) is the ratio of product concentrations to reactant concentrations at equilibrium.
aA + bB cC + dD
From the general equation, each concentration is raised to a power equal to the number of moles of that substance in the balanced chemical equation.
Keq =
[C]c x [D]d
[A]a x [B]b

23. Equilibrium Constants
Write equilibrium constant expressions for the following reactions:
Cl2(g) + I2(g)  2 ICl(g)
2HBr(g)  H2(g)+Br2(g)

24. Chemical Equilibrium
Which of these equations represents a reaction in which entropy decreases?
2MgO(s) → 2Mg(s) + O2(g)
2O3(g) → 3O2(g)
2H2O(l) → 2H2(g) + O2(g)
C(s) + 2H2(g)→ CH4(g)
2NI3(s) → 3I2(g) + N2(g)

25. Acids & Bases
Classify each solution as acidic, basic, or neutral by its pH value.
[H+] = 7.5 x M pH= _______
[H+] = 1.0 x 10-7 M pH= _______
pH = pH= _______
pOH = pH= _______
[OH-] = 2.8 x 10-5 M pH= _______
pH = pH= _______

26. Acids & Bases Arrhenius acid Brønsted-Lowry acid Lewis acid
Arrhenius base
Brønsted-Lowry base
This describes a substance that is a hydrogen-ion acceptor.
This describes a substance that yields hydroxide ions in aqueous solution.
This describes a substance that can accept a pair of electrons to form a covalent bond.

27. Strong Acid Dissociation
Show how nitric acid will ionize or dissociation in water.

28. Ka dissociation
A 0.10M solution of hydrocyanic acid, HCN, has an equilibrium hydrogen ion concentration of 6.3 × 10–6M. What is the Ka of hydrocyanic acid?

29. Potential diagrams
What does this picture represent?